Quiz 3 Flashcards
Density of Gas and Parameters
Density:
Directly Related: Pressure and Molar Mass
Inversely Related: Temperature
Dalton’s Law on Partial Pressure:
P(total) = P(b) + P(a) + P(c) ….
Partial Gas
P(partial gas) = ((n gas)/(n total)) x P(total)
Mole Fraction
Xgas = ngas/ntotal
A gas that makes up 21% of the mixture will contribute ___ % of the total pressure
A gas that makes up 21% (or 0 .21) of a mixture will
contribute 21% of the total pressure.
Kinetic Molecular Theory
-Gases consist of tiny particles that move at various speeds and in every possible direction.
* Most of the volume of a gas is empty space.
* The size of gas particles is much smaller than the distances between them.
* There is no force of attraction or repulsion between gas particles
* Because the particles are so far apart from each other
* All collisions between particles and walls are elastic
* Energy can be transferred between particles during collisions, but none is lost during collisions with walls.
* Kinetic energy is conserved
* Temperature is a measure of the average kinetic energy of the gas particles.
At higher temperatures, gas particles have ____ kinetic energy and move ____.
At higher temperatures, gas particles have more
kinetic energy and move faster.
Temperature and Kinetic Energy:
Temperature is a measure
of the average kinetic
energy of the particles in an object. When temperature
increases, the motion of
these particles also
increases.
Ideal Gas Laws:
An ideal gas consists of particles that have the
following properties:
* Particles have no volume
– They are very small compared to the size of the container.
* Particles exert no forces on each other
– Particles are neither attracted to nor repelled from each
other.
* Kinetic energy is unchanged when gases collide with each other or the walls.
Pressure conversions:
1 atm = 760 mm Hg = 760 torr
Exothermic and Endothermic
releases 483.6 kJ
exothermic
requires 483.6 kJ
endothermic
